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Why solubility of alkaline earth metals decreases down the group?
In my book, it is given that solubility of earth metals increases down the group
$$\ce{BeSO4 > MgSO4 > CaSO4 > SrSO3 > BaSO4}$$
I couldn't really understand how is this possible.
Can anybody explain?
the size (atomic radius) of the element increases. Mg 2+ is a much smaller in size than Ba 2+ because it contains less protons and neutrons in its nucleus. As a result, larger cations form STRONGER bonds with larger anions (CO3 is considered a decent size anion). The rule here is ions of similar size attract one another strongly, and thus do NOT dissociate or become soluble in solution. (used CO3 as example)
